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SOLUTIONS
- a SOLUTION is a HOMOGENEOUS MIXTURE.
Uniform properties throughout!
- parts of a solution:
SOLUTE(S)
- component(s) of a solution present in small amounts.
SOLVENT
- the component of a solution present in the GREATEST amount
- in solutions involving a solid or gas mixed with a LIQUID, the liquid
is typically considered the solvent.
- solutions are usually the same phase as the pure solvent. For example, at
room temperature salt water is a liquid similar to pure water.
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SOLVENTS
- We traditionally think of solutions as involving gases or solids dissolved in liquid solvents. But
ANY of the three phases may act as a solvent!
GAS SOLVENTS
- Gases are MISCIBLE, meaning that they will mix together in any proportion.
- This makes sense, since under moderate conditions the molecules of a gas don't
interact wth each other.
- Gas solvents will only dissolve other gases.
LIQUID SOLVENTS
- Can dissolve solutes that are in any phase: gas, liquid, or solid.
- Whether a potential solute will dissolve in a liquid depends on how compatible the
forces are between the liquid solvent and the solute.
SOLID SOLVENTS
- Solids can dissolve other solids, and occasionally - liquids.
- Solid-solid solutions are called ALLOYS. Brass (15% zinc dissolved in copper) is
a good example.
- AMALGAM is a solution resulting from dissolving mercury into another metal.
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CONCENTRATION
- When you discuss a solution, you need to be aware of:
- what materials are in the solution
- how much of each material is in the solution
- CONCENTRATION is the amount of one substance compared to the others in a solution. This
sounds vague, but that's because there are many different ways to specify concentration!
- We will discuss four different concentration units in CHM 111:
MASS PERCENTAGE
MOLARITY
MOLALITY
MOLE FRACTION
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How would you prepare 455 grams of an aqueous solution that is 6.50% sodium
sulfate by mass?
We know everything in this definition EXCEPT the mass of sodium sulfate we need, so
we calculate the mass of sodium sulfate using basic algebra.
How much water? Subtract the mass of sodium sulfate from the total mass,
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What's the MOLALITY and MOLE FRACTION OF SOLUTE of the previous solution?
previous solution
Convert mass sodium sulfate to moles using formula weight of sodium sulfate.
Convert the 425 g of water to kg
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previous solution
Calculate moles sodium sulfate from the mass using formula weight. (We've
already done this!)
Calculate moles water by converting mass water to moles, then add in
the moles sodium sulfate to get total moles.
(See previous page for calculation)
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MOLARITY
- In the previous example, we converted between three of the four units that we discussed:
mass percent, molality, and mole fraction.
- We didn't do MOLARITY, because the information given in the previous problem was not
sufficient to determine molarity!
1 M NaCl
at 25 C
<1 M NaCl
at 40 C
Molarity is based on VOLUME, while the other three
units are based on MASS. (moles and mass can
be directly converted)
Volume depends on TEMPERATURE!
- If you HEAT a solution, what happens to CONCENTRATION?
... the MOLAR CONCENTRATION decreases. (But the concentration
in the other three units we discussed stays the same.)
- If you COOL a solution, the MOLAR CONCENTRATION increases. (The other three units stay
the same!)
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... we use MOLARITY so much because it's easy to work with. It is easier to measure the VOLUME
of a liquid solution than it is to measure mass.
Example: How would we prepare 500. mL of 0.500 M sodium sulfate in water?
Dissolve the appropriate amount of sodium sulfate into enough water to make 500. mL of
solution.
A VOLUMETRIC FLASK is a flask that
is designed to precisely contain a
certain volume of liquid.
VOLUMETRIC FLASKS are used to
prepare solutions.
volumetric flask
Dissolve 35.5 grams of sodium sulfate in enough water to make 500. mL of
solution. The concentration will be 0.500 M.
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More on MOLARITY
To prepare a solution of a given molarity, you generally have two options:
Weigh out the appropriate amount of solute, then dilute to the desired volume with
solvent (usually water)"
"stock solution"
Take a previously prepared solution of known concentration and DILUTE it with
solvent to form a new solution
- Use DILUTION EQUATION
The dilution equation is easy to derive with simple algebra.
... but when you dilute a solution, the number of moles of solute
REMAINS CONSTANT. (After all, you're adding only SOLVENT)
before
diution
after
dilution
Since the number of moles of solute stays
the same, this equality must be true!
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... the "DILUTION EQUATION"
molarity of concentrated solution
volume of concentrated solution
molarity of dilute solution
volume of dilute solution (TOTAL VOLUME, NOT the volume water added!)
The volumes don't HAVE to be in liters, as long as you use the same volume UNIT for
both
and
Example: Take the 0.500 M sodium sulfate we discussed in the previous example and dilute it
to make 150. mL of 0.333 M solution. How many mL of the original solution will we need to dilute?
Take 99.9 mL of 0.500 M sodium sulfate, and add water until the TOTAL
VOLUME OF THE SOLUTION is 150. mL